3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;0*, CH;CO0 and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x105) CH;COOH(aq) CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;COO- (aq) and H3O* (aq) at equilibrium. c) Calculate pH of the solution.

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3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL
of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at
equilibrium. What is the pH of the solution? (Ka = 1.8x10)
CH;COOH(aq) = CH;COO (aq) + H;O* (aq)
a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16)
b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium.
c) Calculate pH of the solution.
Transcribed Image Text:3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.
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